Can some1 plz tell me that apart from m = Q x e.c.e = density x V, is there another way of finding the thickness of the layer of copper that is deposited on the cathode during electrolysis?

(when u already know the density of Cu, the surface area of the anode, voltmeter and ammeter readings at a particular time and Q).

By the way, i am in grade 12 in QLD, Australia so plz dont tell me something complex learnt from uni. thanx (oh...if u think there isn't or if u know for sure there isn't then can u plz tell me)

The mass of a substance produced at an electrode during electrolysis is proportional to the quantity of electricity that has passed.

 

Look up, Faraday's formula to relate these variables. look at site below:

 

http://www.wpbschoolhouse.btinternet.co.uk/page04/4_73calcs.htm#13.%20Electrolysis%20product

Example 2: How much copper is deposited if a current of 0.2 Amps is passed for 2 hours through a copper(II) sulphate solution ?

Electrode equation: (-) cathode Cu2+(aq) + 2e- ==> Cu(s) and Ar(Cu) = 64

the quantity of electricity passed in Coulombs

= current in A x time in secs (Q = I x t)

= 0.2 x 2 x 60 x 60 = 1440 Coulombs, and 1 mole electrons = 96500 Coulombs

therefore moles of electrons passed through circuit = 1440 / 96500 = 0.01492

it takes two moles of electrons to form one mole of copper

therefore moles copper = 0.01492 7 2 = 0.00746

mass of copper = moles of copper x atomic mass of copper

= 0.00746 x 64 = 0.4775g of copper deposited.

 

Taken from http://www.wpbschoolhouse.btinterne...lysis%20product

ok so if i can find the mass of the copper deposited on the cathode, then to find the thickness of that copper deposited, do i use mass=density x volume...where the volume equals the area of the cathode multiplied by the width of the copper deposited on the cathode? can some1 tell me if that's correct or not?